Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry 101 > Chemical bonding > Flashcards

Chemical bonding Flashcards

You may prefer our related Brainscape-certified flashcards:
Chemistry 101 flashcards Physics 101 flashcards AP® Chemistry flashcards Psychology 101 flashcards Periodic Table flashcards Biology 101 flashcards Organic Chemistry 101 flashcards Sociology 101 flashcards
1
Q

what is a kernel?

A

Kernel: is the nucleus and all inner electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Octet rule

A

An element attain stability by have 8 electrons in its valance shell by sharing or complete transfer of electron

Drawbacks:
1. Element having atomic number less that 4 have unfilled electrons
2. Elements having d orbital are having extended octet
3. Some elements are having odd number of electrons
Noble gases like Xe and Kr form bonds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What was Kossel-Lewis method of representation of atoms?

A

With the symbol of the element and showing its valence shell electron using dots

Drawbacks:
1. didn’t give the shape, nature and energy levels of compound and molecules

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Formal charge

A

method used foe balancing and keeping track of electrons in the molecule

FC = V - L - B
V = valence electrons
L = Lone pair
B = number of bonds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What are the main feature that define an ionic bond?

A

The main feature that define an ionic bond are:
1. Electron gain enthalpy: the energy releases or absorbed when electron is gained
2. Lattice enthalpy: the energy required to break one mole of bond into gaseous ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Why do we need bond parameters?

A

Bond parameters are parameters that help define a bond thus they are important.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

How is bond enthalpy and lattice enthalpy different?

A

Bond enthalpy deals with the amount of energy required to break one mole bond present in gaseous state
where as lattice enthalpy is the energy require to break one mole of bond to give gaseous ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

How is bond length and bond order related ?

A

Bond length is the length between the nuclei of two atoms where as bond order is the number of bond that atom is forming

Bond length increases bond order decreases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Bond angle

A

The angle formed between any two bonds. Depends on the compound

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Resonance

A

Canonical structure: the representation of the same molecule in multiple way. (need one single bond and one double bond)

Resonance: different canonical structure lead to a formation of a hydride where the energy is less and that compound is more stable

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Why is the resonance hybrid more stable that their canonical structures ?

A

This is because the hybrid averages the bond character

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What results in the formation of a polar bonds?

A

Polar bonds are formed due to difference in electronegativity, because of there is is a distortion of electrons towards the more electronegative atoms creating a partials charge

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Dipole moment

A

Charge * distance of separation
it is a vector quantity

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Fajan’s Rules

A

No compound is purely ionic or covalent, they have the properties of both

  1. larger anion and smaller the cation more covalent
  2. more charge on the cation more covalent
  3. more polarizing cation and more polarizability of anion more covalent
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What was the main principle behind the VSEPR theory?

A
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

VSEPR theory

A

Valence shell electron pair repulsion theory
1. the positions acquired in 3-D lead to min repulsion
2. the shape of the compound depends the number of valance electrons
3.Valance shell is considered as a sphere
4.Electron pair repel each other
LP-LP>LP-BP>BP-BP
5. multiple bonds = single electron pair
multiple multiple bonds = super electron pair

17
Q

What kind of geometry does these type of molecules have
1. AB2
2.AB3
3.AB4
4.AB5
6.AB6

A
  1. linear geometry with angle of 180
  2. trigonal planer with angle of 120
    3.Tetrahedral with angle of 109.5
  3. trigonal bipyramidal angle of 90,120
  4. Octahedral with angle of 90,90
18
Q

What kind of structure do these kind of molecules have:
1.Ab2E
2.AB3E
3.AB2E2
4.AB4E
5.AB3E2
6.AB5E
7.AB4E2

A
  1. bent shape with angle of 119.5
    2.trigonal pyramid with angle of 107
  2. bent shape with angle 104.5
  3. Sew saw with angle 90,120
  4. t shaped with angle 90
    6.Squar pyramid
  5. Squar planner
19
Q

Why are axial bonds longer that equatorial bonds?

A

Because axial bond face more repulsion rather that equatorial bonds

20
Q

What is the principle of VBT?

A

Attraction and repulsion between two atoms and molecules

21
Q

What are the result of these attractive and repulsive forces?

A

Due to these attractive and repulsive force there is overlapping of orbitals

22
Q

What is overlapping ?

A

Overlapping means the merging of orbitals
more the over lapping more stronger is the bond

types of overlapping
1. positive overlapping: same signs overlapping
2. negative overlapping: different signs overlapping
3. Zero overlapping: on overlapping at all

23
Q

What are the two types of bond formations?

A
  1. Sigma bond : a bond formed due to head on overlapping of orbitals. It is strong, independent and rotatable
  2. Pi bond: a bond formed due to lateral overlapping of orbitals. They are weak dependent and are not rotatable
24
Q

What is hybridization?

A

The intermixing of atomic orbitals of similar or same energy to form a hybrid orbitals with equivalent energy and shape.

25
Q

Feature of hybridization

A
  1. no. of HO = no of AO
  2. bonds formed are more stable
  3. need to similar energy levels
  4. The orbital need to be half filled
    5.propotion of electron is not necessary
26
Q

What are the different types of hybridisation?

A
  1. sp linear alkyne 50-50
    2.sp2 trigonal planner alkene 33-67
    3.sp3 tetrahedral alkane 25-75
    4.sp2d squar planner
    5.sp3d trigonal pyramid
    6.sp3d2 squar pyramid
27
Q

Feature of MOT

A

Molecular orbital theory
1. no of electrons in Mo = no of electrons is AO
2.similar energy level of AO form MO
3. Influenced by more that one nuclei i.e polycentric
4. types of orbital
a) bonding: less energy, more stable and hold the atoms together
b) anti-bonding: more energy, less stable creates a node between atoms

Overlapping should be done along the same axis and the overlapping need to be max.

28
Q

Energy level diagram for MOT

A
  1. kk(σ2s)(σ2s)(σ2pz)(π2px=π2py)(π2px=π2py)(σ2pz) after nitrogen
  2. kk(σ2s)(σ2s)(π2px=π2py)(σ2pz)(π2px=π2py)(σ2pz) before nitrogen
29
Q

How comes C2 form two pi bonds instead of one pi and one sigma?

A

This is because carbon need 4 electrons to be stable then the formation of two pi bond full fills that

30
Q

Hydrogen bond

A

attractive forces between H and an electronegative element forming a weak bond.
the magnitude of the bond depends on the state in which the sub. is present
S>L>G

31
Q

What are the different types of hydrogen bond

A

There are two different type of hydrogen bond:
1. inter molecule: with another molecule of the same or different compound
2. Intramolecular: within the same molecule between two electronegative elements

Chemistry 101 (9 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions